CHEM 102 2nd Chapter Lecture 7 Outline of Last LectureI. Kineticsa. DefinitionII. Ratea. Definitionb. EquationIII. Collision Theorya. Definitionb. Three thing that must happen for a reaction to occurc. Activation Energyd. Activated ComplexIV. Catalysisa. Definition Outline of Current LectureI. Enzyme Catalysisa. DefinitionII. Chemical Equilibriuma. Definitionb. ExplanationIII. Acids and Basesa. Definitionsb. Weak vs. Strong AcidsThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.c. Properties of Bases and AcidsIV. pH a. Definitionb. How to calculate it and molarityV. Buffersa. DefinitionCurrent LectureEnzyme CatalysisEnzyme Catalysis – large molecules, called macromolecules, which catalyze specific biochemical*They increase the rates of reactions by factors as large as 10 to the 14th * *Very specific in the reactions they catalyze**Very reactive in very mild reaction conditions*Chemical EquilibriumChemical Equilibrium – A state in which the rates of the forward and reverse reactions are equal*It does not mean that both the reactions are equal!!!!*During a Chemical Equilibrium Reaction, the reaction starts going from left to right, but then switches directions. The reaction will go back and forth for a while until the forces from the reaction going in opposite directions offsets each other and the reaction doesn’t move in either direction. IT DOES NOT STOP, IT IS JUST OFFSET BY THE OPPOSITE FORCES COLLIDINGThe principle of Le Chantelier – Any change to a chemical reaction at equilibrium causes the reaction to proceed in the direction that reduces the effects of the change; in other words, if wedo something to upset equilibrium, the direction of the reaction will change to offset the upset. *If you add something to the product of a reaction equation, the direction will change to go towards the reactant and vice versa*Acids and BasesAcid – A substance that releases H+ ions when dissolved in water- Sour Taste- Give off H+ ions- Reacts with metals to give hydrogen- Example: vinegar, tomatoes, citrus fruit, aspirinBase – A substance that releases OH – ions when dissolves in water- Bitter taste- Provides OH-- Slippery feeling- Examples: Ammonia, Baking soda, soap detergents, soap*There are strong acids and bases, and weak acids and bases**Strong acids and bases destroy each other when they react with each other, but when weak acids and bases react with each other, they create equilibrium*Conjugate Acid/Base pairs - Acids donate H+- Bases accept H+Find the Conjugate pairsCH3NH2 + H2O  CH3NH3 + OH- CH3NH2 and CH3NH3 are conjugate acid/base pairs because CH3NH2, the acid, gave away a H+ for it’s pair CH3NH3, which is the base.H2O and OH- are a conjugate acid/base pair because H2O gave a hydrogen, making it an acid, and OH- accepted one, making it a base.Hydronium ion (H3O or H+) – a hydrated protonAcid- base indicators – Substances that change color with the changes in acidity or basicity of a solution*The strength of acids and bases are based on their ability to completely dissociate in water. Strong acids and bases dissociate 100%, but weak acids and bases may only dissociate 15%-20%*MEMORIZE THE TABLE OF STRONG ACIDS AND BASES IN THE NOTES! IF THE ACID OR BASES YOUARE DEALING WITH IS NOT ON THAT LIST, IT IS A WEAK ACID OR BASE!pHpH – numerical measure of the acidity or basicity of a solution. It is the measure of the hydronium ion concentrationTo calculate pH take the negative logarithm of the hydronium ion concentration of a solutionEx.- LOG (.0025) = 2.60Molarity – the number of moles per liter of solutionTo find molarity, take the moles of the substance and divide it by how may liters of solution you have.EX. You have a beaker of 500 ml of a solution and are dissolving 1.5 g of NaOH- into it. First find the moles of NaOH- which is .038. Then find out how many liters of solution you have which is ½of al liter. Take .038/ .500 to get .076 molarity.Buffer – a solution of weak acids or bases and their conjugate partners. Buffers keep a solution from getting too acidic or basic*Things are buffers if they have a conjugate pair and it is a weak acid or